The standard oxidation potentials,${E^ \circ }$ for the half reactions are ; ${\rm{Zn}} \to {\rm{Z}}{{\rm{n}}^{2 + }} + 2e;{E^ \circ } = + 0.76{\rm{V}}$ ${\rm{Ag}} \to {\rm{A}}{{\rm{g}}^ + } + e;{E^ \circ } = - 0.77{\rm{V}}$ The standard e. m. f. of the cell, ${\rm{A}}{{\rm{g}}^ + } + {\rm{Zn}} \to {\rm{Z}}{{\rm{n}}^{2 + }} + {\rm{Ag}}$ is :

NEET UG CHEMISTRY MCQ: ELECTRO CHEMISTRY

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The standard oxidation potentials,

{E^ \circ }

for the half reactions are ;

\mathrm{Zn} \to \mathrm{Z}{\mathrm{n}^{2 + }} + 2e;{E^ \circ } = + 0.76\mathrm{V}

\mathrm{Ag} \to \mathrm{A}{\mathrm{g}^ + } + e;{E^ \circ } = - 0.77\mathrm{V}

The standard e. m. f. of the cell,

\mathrm{A}{\mathrm{g}^ + } + \mathrm{Zn} \to \mathrm{Z}{\mathrm{n}^{2 + }} + \mathrm{Ag}

is :

View answer and explanation

Correct option: A

+ 1.53 V

Option A is correct. The standard EMF of the cell is calculated by adding the standard oxidation potential of the anode (Zn) and the standard reduction potential of the cathode (Ag).

NEET UG CHEMISTRY MCQ: ELECTRO CHEMISTRY

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